1. Chapter 4: Atomic Structure
4.1: Studying Atoms
4.2: The Structure of an Atom
4.3: Modern Atomic Theory

2. 4.1: Studying Atoms
Greeks
Dalton
Thomson
Rutherford
Atomic Model

3. Ancient Greek Models of Atoms
Democritus believed that all matter consisted of extremely small particles that could not be divided.

4. Ancient Greek Models of Atoms
Democritus called these particles atoms from the Greek word atomos, which means “uncut” or “indivisible.”
He thought there were different types of atoms with specific sets of properties

5. Aristotle
Thought that all substances were built up from only four elements.

6. Dalton’s Atomic Theory
Proposed the theory that all matter is made up of individual particles called atoms, which cannot be divided.
Compounds contain atoms of more than on element.
In a particular compound, atoms of different elements always combine in the same way.

7. Dalton’s Experiment
The ratio of the masses of the elements in the compound is always the same.
A 100 gram sample of magnesium combines with 65.8 grams of oxygen.
A 10 gram sample of magnesium combines with 6.58 grams of oxygen.

8. Dalton’s Model
The elements are pictured as solid spheres.

9. Thomson’s Experiment

10. Thomson’s Experiment
Thomson’s experiments provided the first evidence that atoms are made of even smaller particles.

11. Thomson’s Model (plum pudding)
In an atom, the negative charges were evenly scattered throughout an atom filled with a positively charged mass of matter.

12. Rutherford’s Experiment

13. Rutherford’s Gold Foil Experiment

15. Rutherford’s Model
All of an atom’s positive charge is concentrated in its nucleus.
The nucleus is a dense, positively charged mass located in the center of the atom.
Pretending to be Alpha Particles Mv.

16. 4.2:Structure of an Atom
Protons, electrons, and neutrons are subatomic particles.
Because these particles are even smaller than an atom, they are called subatomic particles.
These three types of particles are arranged in an atom as shown below.

17. What makes one element different from another if?
All protons are the same.
All electrons are the same.
All neutrons are the same.

18. Protons
The number of protons distinguishes an atom of one element from the atom of another element.
All atoms of the same element will have the same number of protons, and atoms of different elements will have different numbers of protons.

20. Properties of Subatomic Particles
Protons, electrons, and neutrons can be distinguished by mass, charge, and location in an atom.

21. Atomic Number The number of protons in an atom of that element.
Because the number of protons in an atom remains the same during physical and chemical changes, we can refer to each element by the number of protons its atoms contain. This unique number is called the atomic number.

22. # protons = # electrons Atomic Number
Because atoms have an overall neutral charge, atoms have an equal number of protons & electrons.
# protons = # electrons

23. Mass Number
the sum of the protons and neutrons in the nucleus of that atom.

24. Isotopes
Isotopes
atoms of the same element that have different numbers of neutrons and different mass numbers.

27. 4.3 Modern Atomic Theory
"D'oh!"

28. Bohr’s Atomic Model Focused on the Electrons

29. 1803: John Dalton
Atoms are tiny, indestructible particles, with no internal structure.

30. 1897: JJ Thomson Discovers the electron
He pictures electrons embedded in a sphere of positive electric charge.

31. 1911: Ernest Rutherford
Atoms have a dense, positively charged nucleus.
Electrons move randomly around nucleus.
Gold foil experiment

32. 1913: Niels Bohr
Electrons move in spherical orbits at fixed distances from the nucleus.

33. 1926: Electron Cloud Model
A visual model of the probable locations of electron in an atom.

34. 1932: James Chadwick
Confirms the existence of neutrons in the nucleus.
Neutrons have no charge.